According to the National Institute of Standards webbook,the Henry's Law constant for N2 gas is 0.00060 mol/kg.bar at 25S1U1P1$\circ$S1S1P0C What is the Henry's law constant in units of mol/kg.atm? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

A) mol/kg.atm B) mol/kg.atm C) mol/kg.atm D) mol/kg.atm E) mol/kg.atm A) mol/kg.atm B) mol/kg.atm C) mol/kg.atm D) mol/kg.atm E) mol/kg.atm A

Henry's Law constant is 0.034 mol/kg.bar and 0.0013 mol/kg.bar for CO2 and O2 respectively at 25S1U1P1$\circ$S1S1P0C.What pressure of O2 is required to achieve the same solubility as 0.218 bar of CO2?

A) 5.7 bar B) 0.0083 bar C) bar D) bar E) 0.18 bar A) 5.7 bar B) 0.0083 bar C) bar D) bar E) 0.18 bar

The Henry's law constant for O2 in water at 25 S1U1P1$\circ$S1S1P0C is 1.3 $\times$ 10-3 mol/kg.bar.What partial pressure of O2 (in atm)is necessary to achieve an equilibrium concentration of 2.9 $\times$ 10-3 mol/kg O2? (1 atm = 0.9869 bar)

A) 0.44 atm B) 0.45 atm C) 2.1 atm D) 2.3 atm E) 3.8 atm A) 0.44 atm B) 0.45 atm C) 2.1 atm D) 2.3 atm E) 3.8 atm

What mass of ethylene glycol,when mixed with 225 g H2O,will reduce the equilibrium vapor pressure of H2O from 1.00 atm to 0.800 atm at 100 S1U1P1$\circ$S1S1P0C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol,respectively.Assume ideal behavior for the solution.

A) 15.6 g B) 49.9 g C) 194 g D) 969 g E) 3.10 $\times$ 103 g A) 15.6 g B) 49.9 g C) 194 g D) 969 g E) 3.10 $\times$ 103 g

What is the vapor pressure at 20°C of an ideal solution prepared by the addition of 4.60 g of the nonvolatile solute urea,CO(NH2)2,to 50.2 g of methanol,CH3OH? The vapor pressure of pure methanol at 20°C is 89.0 mmHg.

A) 4.15 mmHg B) 76.0 mmHg C) 81.5 mmHg D) 84.9 mmHg E) 13.0 mmHg A) 4.15 mmHg B) 76.0 mmHg C) 81.5 mmHg D) 84.9 mmHg E) 13.0 mmHg

If the concentration of sodium carbonate in water is 12.8 ppm,what is the molarity of Na2CO3(aq)? The molar mass of Na2CO3 is 106.0 g/mol.Assume the density of the solution is 1.00 g/mL.

A) 8.28 $\times$ 10-6 M B) 1.21 $\times$ 10-4 M C) 1.36 $\times$ 10-3 M D) 0.136 M E) 0.121 M A) 8.28 $\times$ 10-6 M B) 1.21 $\times$ 10-4 M C) 1.36 $\times$ 10-3 M D) 0.136 M E) 0.121 M

If 27.9 g LiCl is dissolved in 175 g H2O,what is the weight percent of LiCl in the solution?

A) 0.376% B) 6.78% C) 13.8% D) 15.9% E) 19.0% A) 0.376% B) 6.78% C) 13.8% D) 15.9% E) 19.0%

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of O2, O2(g)$\leftrightarrows$O2(aq) What is the effect on the equilibrium composition of the liquid when the $\underline{\text{ temperature }}$ of the liquid is decreased?

A) The amount of O2 dissolved in the liquid decreases. B) The amount of O2 dissolved in the liquid increases. C) The amount of O2 dissolved in the liquid does not change. D) Not enough information is provided to answer the question. E) Either A or B could occur. A) The amount of O2 dissolved in the liquid decreases. B) The amount of O2 dissolved in the liquid increases. C) The amount of O2 dissolved in the liquid does not change. D) Not enough information is provided to answer the question. E) Either A or B could occur.

Which of the following liquids will be miscible with water in any proportion: ethanol (CH3CH2OH),carbon tetrachloride (CCl4),hexane (C6H14),and/or formic acid (HCO2H)?

A) ethanol and carbon tetrachloride B) carbon tetrachloride and hexane C) ethanol and formic acid D) ethanol,carbon tetrachloride,and benzene E) carbon tetrachloride,and formic acid A) ethanol and carbon tetrachloride B) carbon tetrachloride and hexane C) ethanol and formic acid D) ethanol,carbon tetrachloride,and benzene E) carbon tetrachloride,and formic acid

Exam 14: Solutions and Their Behavior

According to the National Institute of Standards webbook,the Henry's Law constant for N₂ gas is 0.00060 mol/kg.bar at 25^$\circ$C What is the Henry's law constant in units of mol/kg.atm? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

Free

(Multiple Choice)

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Question 1

Correct Answer:

Verified

Which of the following solutions would have the highest osmotic pressure?

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(Multiple Choice)

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Question 2

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Verified

The vapor pressure of water at 90°C is 0.692 atm.What is the vapor pressure (in atm)of a solution made by dissolving 1.28 mole(s)of CsF(s)in 1.00 kg of water? Assume that Raoult's law applies.

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

Henry's Law constant is 0.034 mol/kg.bar and 0.0013 mol/kg.bar for CO₂ and O₂ respectively at 25^$\circ$C.What pressure of O₂ is required to achieve the same solubility as 0.218 bar of CO₂?

(Multiple Choice)

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Question 4

________ are colloidal dispersions of one liquid in another liquid.

(Short Answer)

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Question 5

The Henry's law constant for O₂ in water at 25 ^$\circ$C is 1.3 $\times$ 10^-3 mol/kg.bar.What partial pressure of O₂ (in atm)is necessary to achieve an equilibrium concentration of 2.9 $\times$ 10^-3 mol/kg O₂? (1 atm = 0.9869 bar)

(Multiple Choice)

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Question 6

Two nonpolar solvents,such as hexane and carbon tetrachloride,may be miscible even though the enthalpy of mixing of these liquids might be small.A reason that mixing occurs is that mixtures have a greater dispersal of energy relative to pure solvents.The tendency toward greater dispersal of energy is a thermodynamic function called ____.

(Multiple Choice)

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Question 7

Assuming ideal behavior,which of the following aqueous solutions should have the highest boiling point?

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Question 8

What mass of ethylene glycol,when mixed with 225 g H₂O,will reduce the equilibrium vapor pressure of H₂O from 1.00 atm to 0.800 atm at 100 ^$\circ$C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol,respectively.Assume ideal behavior for the solution.

(Multiple Choice)

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Question 9

The change in energy accompanying the process below is the ____ of MX. MX(s) $\to$ M⁺(aq)+ X^-(aq)

(Multiple Choice)

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Question 10

What is the vapor pressure at 20°C of an ideal solution prepared by the addition of 4.60 g of the nonvolatile solute urea,CO(NH₂)₂,to 50.2 g of methanol,CH₃OH? The vapor pressure of pure methanol at 20°C is 89.0 mmHg.

(Multiple Choice)

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Question 11

If the concentration of sodium carbonate in water is 12.8 ppm,what is the molarity of Na₂CO₃(aq)? The molar mass of Na₂CO₃ is 106.0 g/mol.Assume the density of the solution is 1.00 g/mL.

(Multiple Choice)

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Question 12

If 27.9 g LiCl is dissolved in 175 g H₂O,what is the weight percent of LiCl in the solution?

(Multiple Choice)

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Question 13

For the following gas-liquid equilibrium for an aqueous system at a constant partial pressure of O₂, O₂(g) $\leftrightarrows$ O₂(aq) What is the effect on the equilibrium composition of the liquid when the $\underline{\text{ temperature }}$ of the liquid is decreased?

(Multiple Choice)

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Question 14

What type of colloid is formed when a solid is dispersed in a liquid?

(Multiple Choice)

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Question 15

At 37°C,what is the osmotic pressure of a 0.59% NaCl by weight aqueous solution? Assume the density of the solution is 1.0 g/mL.Assume no ion pairing.(R = 0.0821 L · atm/K·mol)

(Multiple Choice)

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Question 16

Which of the following liquids will be miscible with water in any proportion: ethanol (CH₃CH₂OH),carbon tetrachloride (CCl₄),hexane (C₆H₁₄),and/or formic acid (HCO₂H)?

(Multiple Choice)

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Question 17

Which of the following statements about soaps and detergents is $\underline{\text{ false? }}$

(Multiple Choice)

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Question 18

Concentrated sodium hydroxide is 19.4 M and has a density of 1.54 g/mL.What is the molality of concentrated NaOH?

(Multiple Choice)

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Question 19

Ideally,colligative properties depend only on the

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Question 20

Showing 1 - 20 of 83

Exam 14: Solutions and Their Behavior

According to the National Institute of Standards webbook,the Henry's Law constant for N2 gas is 0.00060 mol/kg.bar at 25 ∘\circ∘ C What is the Henry's law constant in units of mol/kg.atm? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

Which of the following solutions would have the highest osmotic pressure?

The vapor pressure of water at 90°C is 0.692 atm.What is the vapor pressure (in atm)of a solution made by dissolving 1.28 mole(s)of CsF(s)in 1.00 kg of water? Assume that Raoult's law applies.

Henry's Law constant is 0.034 mol/kg.bar and 0.0013 mol/kg.bar for CO2 and O2 respectively at 25 ∘\circ∘ C.What pressure of O2 is required to achieve the same solubility as 0.218 bar of CO2?

________ are colloidal dispersions of one liquid in another liquid.

The Henry's law constant for O2 in water at 25 ∘\circ∘ C is 1.3 ×\times× 10-3 mol/kg.bar.What partial pressure of O2 (in atm)is necessary to achieve an equilibrium concentration of 2.9 ×\times× 10-3 mol/kg O2? (1 atm = 0.9869 bar)

Assuming ideal behavior,which of the following aqueous solutions should have the highest boiling point?

What mass of ethylene glycol,when mixed with 225 g H2O,will reduce the equilibrium vapor pressure of H2O from 1.00 atm to 0.800 atm at 100 ∘\circ∘ C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol,respectively.Assume ideal behavior for the solution.

The change in energy accompanying the process below is the ____ of MX. MX(s) →\to→ M+(aq)+ X-(aq)

What is the vapor pressure at 20°C of an ideal solution prepared by the addition of 4.60 g of the nonvolatile solute urea,CO(NH2)2,to 50.2 g of methanol,CH3OH? The vapor pressure of pure methanol at 20°C is 89.0 mmHg.

If the concentration of sodium carbonate in water is 12.8 ppm,what is the molarity of Na2CO3(aq)? The molar mass of Na2CO3 is 106.0 g/mol.Assume the density of the solution is 1.00 g/mL.

If 27.9 g LiCl is dissolved in 175 g H2O,what is the weight percent of LiCl in the solution?

What type of colloid is formed when a solid is dispersed in a liquid?

At 37°C,what is the osmotic pressure of a 0.59% NaCl by weight aqueous solution? Assume the density of the solution is 1.0 g/mL.Assume no ion pairing.(R = 0.0821 L · atm/K·mol)

Which of the following liquids will be miscible with water in any proportion: ethanol (CH3CH2OH),carbon tetrachloride (CCl4),hexane (C6H14),and/or formic acid (HCO2H)?

Which of the following statements about soaps and detergents is false? ‾\underline{\text{ false? }} false? ​

Concentrated sodium hydroxide is 19.4 M and has a density of 1.54 g/mL.What is the molality of concentrated NaOH?

Ideally,colligative properties depend only on the

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According to the National Institute of Standards webbook,the Henry's Law constant for N₂ gas is 0.00060 mol/kg.bar at 25^$\circ$C What is the Henry's law constant in units of mol/kg.atm? (1 bar = 0.9869 atm; 1 atm = 760 mmHg)

Henry's Law constant is 0.034 mol/kg.bar and 0.0013 mol/kg.bar for CO₂ and O₂ respectively at 25^$\circ$C.What pressure of O₂ is required to achieve the same solubility as 0.218 bar of CO₂?

The Henry's law constant for O₂ in water at 25 ^$\circ$C is 1.3 $\times$ 10^-3 mol/kg.bar.What partial pressure of O₂ (in atm)is necessary to achieve an equilibrium concentration of 2.9 $\times$ 10^-3 mol/kg O₂? (1 atm = 0.9869 bar)

What mass of ethylene glycol,when mixed with 225 g H₂O,will reduce the equilibrium vapor pressure of H₂O from 1.00 atm to 0.800 atm at 100 ^$\circ$C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol,respectively.Assume ideal behavior for the solution.

The change in energy accompanying the process below is the ____ of MX. MX(s) $\to$ M⁺(aq)+ X^-(aq)

What is the vapor pressure at 20°C of an ideal solution prepared by the addition of 4.60 g of the nonvolatile solute urea,CO(NH₂)₂,to 50.2 g of methanol,CH₃OH? The vapor pressure of pure methanol at 20°C is 89.0 mmHg.

If the concentration of sodium carbonate in water is 12.8 ppm,what is the molarity of Na₂CO₃(aq)? The molar mass of Na₂CO₃ is 106.0 g/mol.Assume the density of the solution is 1.00 g/mL.

If 27.9 g LiCl is dissolved in 175 g H₂O,what is the weight percent of LiCl in the solution?

Which of the following liquids will be miscible with water in any proportion: ethanol (CH₃CH₂OH),carbon tetrachloride (CCl₄),hexane (C₆H₁₄),and/or formic acid (HCO₂H)?

Which of the following statements about soaps and detergents is $\underline{\text{ false? }}$